What is the wavelength of the light emitted when the electron in a hydrogen atom undergoes transition from the energy level with n = 4 to energy level n = 2? What is the colour corresponding to this wavelength? (Given R_H = 109678 cm^-1)

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Payal Gupta | Contributor-Level 10

9 months ago

According to Balmer formula,

Wave number (? ) = R_H [1/n₁²- 1/n₂²]cm^-1

= 109678 [1/2² – 1/4²] cm^-1

= (109678 x 3) / 16 cm^-1

λ = 1 /? = 16 / (109678 x 3) cm = 16 x 10⁷ / (109678 x 3) nm = 486 nm

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What is the wavelength of the light emitted when the electron in a hydrogen atom undergoes transition from the energy level with n = 4 to energy level n = 2? What is the colour corresponding to this wavelength? (Given RH = 109678 cm-1)